Respuesta :
Answer:
final mole fraction of O₂ = 58.84% , CO₂ = 17.64% , H₂O = 23.52% .
final partial pressure of O₂ = 2.942 atm , CO₂ = 0.882 atm , H₂O = 1.176 atm .
Explanation:
Assuming that propane is present as a gas , and also that the combustion is complete:
C₃H₈ + 5 O₂ → 3 CO₂ + 4 H₂O
then taking as a reference propane sample= 1 mol , then
initial moles of O₂ = 3* 5 moles = 15 moles
final moles of O₂= 3* 5 moles - 5 moles = 10 moles
final moles of CO₂ = 3 moles
final moles of H₂O = 4 moles
total number of moles = 10 + 3 + 4 = 17 moles
final mole fraction of O₂ = 10/17 = 0.5884 = 58.84%
final mole fraction of CO₂ = 3/17 = 0.1764 = 17.64%
final mole fraction of H₂O = 4/17 = 0.2352 = 23.52%
From Dalton's law for ideal gases , the partial pressure p=P*x then
final partial pressure of O₂ = 5 atm * 10/17 = 2.942 atm
final partial pressure of CO₂ = 5 atm * 3/17 = 0.882 atm
final partial pressure of H₂O = 5 atm * 1/17 = 1.176 atm
Answer:
Mol fraction CO2 = 0.176
Mol fraction H2O = 0.235
Mol fraction O2 = 0.588
Partial pressure of CO2 = 0.88 atm
Partial pressure of H2O = 1.175 atm
Partial pressure of O2 = 2.94 atm
Explanation:
Step 1: Data given
amount of O2 = 3 times the amount needed to completely oxidize propane
Step 2: The balanced equation:
C3H8 + 5 O2 → 3 CO2 + 4 H2O
Step 3: Calculate moles at the start
Suppose there is 1.00 mol of C2H8 to start.
Then there is 1.00 * 5 *3.00 = 15.0 moles of O2 to start.
Step 4: Calculate moles at the equilibrium
After the reaction,1.00 mol of C3H8 is completely consumed
There is 3*1.00 = 3.00 moles of CO2 and 4*1.00 = 4.00 moles H2O moles produced
There will be consumed 5*1.00 = 5.00 moles of O2
There will remain 15.00 - 5.00 = 10.00 moles O2
Step 5: Calculate total moles of gases at the end
Total moles of gases at the end: 3 moles CO2 + 4 moles H2O + 10 moles O2 = 17.0 moles
Step 6: Calculate mol fraction
Mol fraction CO2 = 3.00 moles / 17.00 moles = 0.176
Mol fraction H2O = 4.00 moles / 17.00 moles = 0.235
Mol fraction O2 = 10.00 moles / 17.00 moles = 0.588
Mol fraction CO2 + mol fraction H2O + mol fraction O2 = 0.176 + 0.235 + 0.588 = 1
Step 7: Calculate partial pressure
Partial pressure of CO2 = 0.176 * 5.00 atm = 0.88 atm
Partial pressure of H2O = 0.235 * 5.00 atm = 1.175 atm
Partial pressure of O2 = 0.588 * 5.00 atm = 2.94 atm
Partial pressure of CO2 + partial pressure of H2O + partial pressure of O2 = 0.88 atm + 1.175 atm + 2.94 atm = 5 atm
